Shape of `Fe(CO)_(5)` is

Options

A. Octahedral
B. Square planar
C. Trigonal bipyramidal
D. Square pyramidal

Answer

To determine the shape of `Fe(CO)_(5)`, we can follow these steps:

### Step 1: Identify the Coordination Number
The coordination number of a metal complex is determined by the number of ligands attached to the central metal atom. In `Fe(CO)_(5)`, there are five CO ligands coordinated to the iron (Fe) atom.

**Hint:** The coordination number is simply the number of ligands surrounding the central metal atom.

### Step 2: Determine the Hybridization
The hybridization of the central metal atom can be determined using the formula:
\[ \text{Hybridization} = \text{Number of bond pairs} + \text{Number of lone pairs} \]

In `Fe(CO)_(5)`, there are five CO ligands and no lone pairs on the iron atom. Therefore:
\[ \text{Hybridization} = 5 + 0 = 5 \]

This corresponds to `sp^3d` hybridization.

**Hint:** Count the number of bonds and lone pairs to find the hybridization.

### Step 3: Predict the Geometry
The geometry associated with `sp^3d` hybridization is trigonal bipyramidal. In this arrangement, three ligands are positioned in a plane (equatorial position), while the other two ligands are above and below this plane (axial position).

**Hint:** Different hybridizations correspond to specific geometries; `sp^3d` corresponds to a trigonal bipyramidal shape.

### Step 4: Conclusion
Thus, the shape of `Fe(CO)_(5)` is trigonal bipyramidal.

**Final Answer:** The shape of `Fe(CO)_(5)` is trigonal bipyramidal.